CHAPTER 7: PERIODIC PROPERTIES OF THE ELEMENTS

Tellurium

________ is a metalloid, and polonium, which is radioactive and quite rare, is a metal.

Fluorine

________ and chlorine are more reactive than bromine and iodine.

Coulombs law

________ tells us that the strength of the interaction between two electrical charges depends on the magnitudes of the charges and on the distance between them.

Solids

________ are usually brittle; some are hard, and some are soft.

pure silicon

Very ________ is an electrical insulator, but its conductivity can be dramatically increased with the addition of specific impurities called dopants.

oxides

Most nonmetal ________ are acidic, which means that those that dissolve in water form acids.

single atoms

They are all monatomic (that is, they consist of ________ rather than molecules)

Oxygen

________ is a colorless gas at room temperature; all of the other members of group 6A are solids.

Anions

________ are larger than their parent atoms.

Metals

________ tend to have low ionization energies and therefore tend to form cations relatively easily.

valence electrons

The ________ added to counterbalance the increasing nuclear charge screen one another ineffectively.

ionization energy

Increased radius decreases nucleus- electron attraction, lowering ________.

Chlorine

________ is the most industrially useful of the halogens.

Compounds

________ made up of a metal and a nonmetal tend to be ionic substances.

Hydrogen

________ is a nonmetal that occurs as a colorless diatomic gas, H2 (g), under most conditions.

molecular substances

Most nonmetal oxides are ________ that form acidic solutions.

atomic weight

When elements are grouped by ________, identical chemical and physical properties occur periodically.

sharp increase

The ________ in ionization energy that occurs when an inner- shell electron is removed.

ionic halides

The halogens react directly with most metals to form ________.

nuclear charge increases

In any isoelectronic series, we can list the members in order of increasing atomic number; therefore, the ________ as we move through the series.

Neil Bartlett

In 1962, ________ (1932- 2008) at the University of British Columbia reasoned that the ionization energy of Xe might be low enough to allow it to form compounds.

Ionic compounds

________ can be used to calculate ionic radii from interatomic distances, much like molecules can.

isoelectronic series

A(n) ________ is a group of ions all containing the same number of electrons.

Metals

________ are shiny, malleable, and ductile.

Solids

________ are malleable and ductile.

Oxygen

________ has a great tendency to attract electrons from other elements (to oxidize them)

alkali metals

The ________ are soft metallic solids.